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Question
The solubility of AgCl(s) with solubility product 1.6 × 10−10 in 0.1 M NaCl solution would be ____________.
Options
1.26 × 10−5 M
1.6 × 10−9 M
1.6 × 10−11 M
Zero
Solution
The solubility of AgCl(s) with solubility product 1.6 × 10−10 in 0.1 M NaCl solution would be 1.6 × 10−9 M.
Explanation:
\[\ce{AgCl_{(s)} ⇌ Ag^+_{( aq)} + Cl^-_{( aq)}}\]
\[\ce{\underset{0.1 M}{NaCl} -> \underset{0.1 M}{Na^+} + \underset{0.1 M}{Cl^-}}\]
Ksp = 1.6 × 10−10
Ksp = [Ag+] [Cl–]
Ksp = (S) (S + 0.1)
0.1 > > > S
∴ S + 0.1 ≃ 0.1
∴ S = `(1.6 xx 10^-10)/0.1`
= 1.6 × 10−9
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